Chemistry 1B General Chemistry Laboratory Manual Spring 2011
Chemistry 1BGeneral ChemistryLaboratory ManualSpring 201121
Table of ContentsLaboratory Policies and Regulations2Laboratory Notebook Requirements and Tips6Review of Nomenclature10Experiment 1 Chemical Reactions and Net Ionic Equations14Experiment 2 Standardization of Sodium Hydroxide Solution28Experiment 3 Acid-Base Titration35Experiment 4 Titration Curves for Polyprotic Acids44Experiment 5 Acids, Bases, and Buffers52Experiment 6 Solubility Product Constant for Calcium Sulfate65Experiment 7 Qualitative Analysis: Anions71Experiment 8 Qualitative Analysis of Silver and Barium-Mg78Experiment 9 Determination of Enthalpy and Entropy Changes83Experiment 10 Electrochemistry88Experiment 11 Sulfide Separations99Experiment 12 Separation and Identification Using Paper Chrom. 104Experiment 13 Cis and Trans K[Cr(H2O)2(C2O4)2]110Experiment 14 Coordination Complexes of Co(III)116Experiment 15 Preparation of Organic Compounds125Appendices1281
California State University, SacramentoDepartment of ChemistryLaboratory PoliciesI. SAFETYa. Familiarize yourself with the location and use of all safety equipment andemergency exits in the laboratory.b. Eating and drinking are not allowed in the laboratory at any time.c. Visitors are not allowed in the laboratory; leave the room for the duration of thevisit.d. YOU MUST: Wear department approved safety goggles at all times when in lab. Shieldsare never allowed! Wear shoes that completely cover your foot when in lab. Wear appropriate clothing that covers your skin or wear a lab coat when inlab. Long hair must be restrained to prevent fire hazard.e. For chemical spills On your skin rinse the area thoroughly for at least 15 min and reportincident to your instructor and the stockroom. For splashes into the eyes rinse using an eyewash for at least 15 minutes,and notify your instructor and the stockroom.f. Working in laboratories outside of the regularly scheduled periods is stronglydiscouraged. When such work is necessary, the written permission of bothinstructors is REQUIRED.g. Students in lower division laboratories are not to work in the laboratory unless aninstructor is immediately available (i.e. in the lab).h. Students in upper division laboratories are not to work in the laboratory unless aninstructor is available in the vicinity (i.e. on the floor).i. Experiments using utilities such as gas, water, steam, heat, etc. are not to be leftunattended. If it is necessary to use these utilities overnight, you must attach a cardsigned by your instructor to the apparatus and notify the Chemistry Stockroom.j. Broken glassware must be placed in the "glass disposal boxes" provided.k. Unauthorized experimentation is prohibited!l. NO CHEMICALS, SUPPLIES, OR EQUIPMENT ARE TO BE REMOVEDFROM THE LABORATORY WITHOUT THE WRITTEN PERMISSIONOF THE INSTRUCTOR AND THE STOCKROOM SUPERVISOR.II. PREGNANCYa. Women that are, or may become pregnant should carefully determine, uponconsultation with your personal physician or the Student Health Service Center, if itis advisable for them to participate in the laboratory program. If you are pregnant orare planning to become pregnant please inform your instructor.2
III. CHEMICALSa. Treat all chemicals as if they were hazardous.b. It is the student's responsibility to know the hazards of the chemicals used in the lab.This information is located in the chemical's MSDS (material safety data sheet),which can be obtained from the kiosks at the north end of the 4th and 5th floors ofSequoia Hall.c. Students are encouraged to practice good chemical hygiene by washing their handsafter lab, and before eating, drinking or smoking.d. Never put chemical waste down drains or in the trash receptacles. Use appropriatelylabeled waste containers.e. If a chemical waste container is almost full, immediately notify your instructor or theStockroom. DO NOT OVERFLOW THE WASTE CONTAINER!f. Never put anything (i.e. spatulas, pipets, fingers, etc.) into a reagent bottle. Place anyunused reagents in the appropriate waste container; DO NOT return it to the bottle.g. Always return chemicals to their appropriate location.h. NEVER remove or borrow chemicals from another laboratory.i. If a required chemical is not available or needs to be refilled, notify your instructor.j. If chemicals are spilled, clean up the mess immediately. This especially includesspill on or around balances and other equipment. If you are unsure of how to cleanup a spill, seek assistance from your instructor or the Stockroom.IV. EQUIPMENTa. DO NOT use any equipment until you have been properly instructed in its use.b. DO NOT move ANY piece of equipment without the permission of your instructor.c. DO NOT attempt to alter or repair any piece of equipment. If it is not in properworking order, inform your instructor.d. Clean all equipment immediately after you have finished using it, and if it wasborrowed or checked out, return it immediately.e. Because of the limited number of certain items. Special equipment issued by theStockroom must be returned the same day or a fine of 5.00 will be assessed.V. STOCKROOMa. The Chemistry Stockroom staff WILL NOT issue chemicals or equipment (otherthan those specifically listed for an experiment, student locker or instructionallaboratory) without the consent of the instructor.b. The Stockroom staff WILL NOT set-up labs after they have been taken down. It isbest not to miss your regularly scheduled lab time.VI. EMERGENCIESa. In the event of ANY EMERGENCY, notify your instructor, and the Stockroompersonnel immediately! Dial 911 for emergencies, or 8-6851 to reach campus policeon any campus phone. Emergency phones are located in the lobbies of each floor inSequoia Hall.**Failure to follow these policies will result in your removal from lab!3
Safety ContractI HAVE READ ALL OF THE ABOVE, AND I AGREE TO CONFORM TOITS CONTENTS.Name:Course:Student ID:Section:Signature:Room:Date:Lab Instructor:4
Laboratory Regulations1.Safety is a prime requisite for laboratory work. Eye protection is required at all timesunless explicitly stated otherwise. You can not work without appropriate eye protection. A labapron or coat will prove a good investment for protecting clothing. Learn the location of thesafety equipment: fire extinguisher, safety shower, and eye wash fountain. Injuries/accidentsshould be immediately reported to your instructor.2. Lab work is to be done on an individual basis unless you are instructed otherwise. Prepare forlab by reading the experiment, preparing tables in your lab notebook for collecting data, andcompleting the prelaboratory assignment.3. Record your results immediately and directly into your notebook. Record observations indetail. Do not write on scratch paper, only write in your laboratory notebook.4. The most productive research demands original work, and this is strongly encouraged.However, for safety reasons this may be done only with the approval and supervision of theinstructor. Unauthorized experiments are strictly forbidden.5. Students are allowed in the laboratories only during regularly scheduled class periods. Makeup labs must be approved by the lab instructor and must be completed within one week of themissed laboratory experiment. Approval is usually only given for medical reasons. You maynot work in another lab without written permission from your laboratory instructor and thelaboratory instructor in charge.6. Keep your lab area clean. Wipe up in a safe and approved manner spilled materials. Onlysoluble, harmless materials should be put in the sink, and these should be washed down withplenty of water. Your instructor will advise you when it is permissible to dispose of chemicals inthe sink. Unless otherwise instructed insoluble or toxic materials should be put in the containersprovided for chemical wastes in the hood. If in doubt, do not pour a substance down the drain; itwill soon be carried to a water-treatment plant and possibly pass through into a stream. Heed thewarnings on the reagent bottles. If in doubt ask your instructor.7. Balances and other delicate instruments require special care. Follow carefully the directionsfor their use.5
Laboratory Notebook RequirementsYou must have a notebook for recording laboratory data that meets one of the two followingformats: A lab notebook containing bound pages for original recording of data followed byanother page that has a carbon to make a copy (our bookstore sells the most convenient type).Always begin an experiment on a new page. Each page of an experiment must show thefollowing at the top of the page: (1) Title of experiment; (2) your name; (3) date of activity; and(4) name of partner, if an experiment is done with one.The first item of a new laboratory experiment is a statement of the objective or purpose ofthe experiment (one or two sentences).This is immediately followed by a reference to procedures by referencing page numbers in thelab manual.The second item contains answers to the pre-lab section. Identify this section. You mustclearly answer questions, provide explanations for your answers and include units in all steps ofcalculations.The major section after pre-lab material contains the observations or results for the experiment.This section includes documentation of all observations of results associated with eachprocedure, tables, drawings, and anything else related to the experiment. It is a key part of thelaboratory report and a lack of organization, details, vagueness, etc. will result in low lab scores.All entries in the notebook must be in ink. Record data as you gather them directly into thenotebook. Never record data on loose slips of paper (e.g. paper towels, scrap paper, etc.) forlater transfer to the notebook. Should a correction be necessary, draw a single, light line throughthe erroneous value and enter the correct value (example.) The original value must remainlegible (you may later decide to use it). Wherever possible, tables of data are preferred toisolate values; in either case, all values must be clearly labeled so that your notebook iscomprehensible to someone with training comparable to you own.Data should be neatly organized. Record the measurements at the time you make them. Ifrepeated trials are made, list repetitive measurements in parallel columns. For example:Title of Table (Descriptive)Trial 2Description of what is being recorded Trial 1(units)(units)Trial 3(units)Be sure to include units with all measured numbers. Units are shown in the columns with theirlabels and not with the number.Bring your laboratory notebook and laboratory syllabus to each class period unlessotherwise stated.6
Tips for Successful Report WritingChem 1BEach experiment that you perform will have its own list of information that needs to beorganized into the report you will turn in to your laboratory instructor. This information isfound at the end of each experiment in the section labeled Laboratory Report.General Requirements for each report:All reports are computer processed. Title page: Your title page is always to be typed. Any additional information listedin the Laboratory Report section for Title Page should also be included. Forexample, your partner’s name (if any), the identity of an unknown, etc. Title pageshould always include experiment number, title, your name, section number, anddate. Tables: Any tables that are mentioned in the Laboratory Report section should becomputer processed. There may be an example shown of how that table shouldlook, if not you should create one of your own to display the values or data that isrequested. Generally speaking, re-typing of data collected in lab in not necessaryunless specifically requested the Laboratory Report section. Tables should beformatted in a way that the data/values are clearly presented. This may mean thatyou have to print them in landscape orientation rather than portrait. It depends on thesize of the table, use your judgment and resize columns as necessary. The sampletables below show you an acceptable table with proper sizing and super andsubscripts. The second table shows improper column sizing and font formatting.Acceptable:Ka (exp) H3PO41.79 x 10-5Not Acceptable: Ka (exp)H3PO41.79 x 10 5Your tables should not be split in half; one page and a couple orphaned rows on the nextpage. Reformat your page size (margins) so that it all appears on one page. If a table istoo large to appear on one page, the column headings should be repeated on the second7
page where the table continues. An unacceptable table is shown below and continuesonto the next page without proper column headings:Acid pH obspH theo% DissKa expKa ---------- PAGE BREAK Cl#.##NH4Cl -#.##------#.##Sample Calculations: (hand write) Sample Calculations: Many tables that you prepare will be filled with values thatyou have calculated. See hypothetical table above. You do not need to type a samplecalculations. Neatly hand writing that calculation under the table is sufficient.Remember that if we can’t read it, we can’t grade it. The sample calculationsshould always be shown under the table that displays those values. If thosecalculations cannot be written under the table, clearly list (by giving the pagenumber) where those calculations can be found and number the pages of yourreport (by hand) so that finding them is clearly mapped out. Most students,however, turn in all their calculations so that simple math mistakes can be trackedeasily and fewer points taken off for those mistakes. Questions and Error Analysis: Many experiments you perform this semester willinclude a few questions to be answered. These questions should be typed. Makesure you write in complete sentences. Hint: students often misread or misunderstandthe question being asked. Always re-read what the question is asking you to answer.A common, yet unacceptable answer is shown below:Will the calculated value of K be too high or too low if:1) the original solution was supersaturated?Student answer: if the solution was supersaturated then that means there was toomuch of the solid in the solution. Our calculated value of K will be off a lot becausewe can’t account for this amount.Student did not answer the question that was asked. “Our calculations will be off” isobvious and true for all error analyses yet it does not answer the question asked.Make sure you answer the question you are asked. Conclusions: Some experiments ask you to reflect and make conclusions at the endabout what you have done. Conclusions should be typed. A one sentence conclusionis never sufficient however a full page is rarely needed either. Generally a paragraphis all that is needed to accurately describe your conclusions.8
Pre-Lab Assignment: Always include your prelab assignment (yellow copies unlessunreadable). You can put your prelab with all corrections made at the beginning ofthe report or at the end. Corrections can be made in your lab notebook or on aseparate piece of paper, it is your choice. As always, please make those correctionseasy to read and reference where those corrections can be found (by page # inreport) if they are placed elsewhere in the report.Data Pages: yellow copy pages unless unreadable, inwhich case you shouldmake photocopies to attach. Thank you: We know how hard you work in this class, thank you for all your hardwork! 9
Nomenclature of Acids, Bases and SaltsReviewI. Objective: To review the rules for naming common inorganic acids, bases and salt.II. Principles: The rules of nomenclature are the rules published by the InternationalUnion of Pure and Applied Chemistry (IUPAC). Compounds are still named by theserules; however, others are still named by their historical names (common names). Therules in this section are used by chemists in naming acids, bases and simple salts derivedfrom acids and bases.I. Binary Compounds.A binary compound contains only two elements. In general, a binary compound isnamed by first stating the name of the more electropositive element, followed by the nameof the more electronegative element (usually a nonmetal), changing its stem to -ide.A. Acids: Binary acids in aqueous solution are named differently than in the gas phase.Refer to the examples below to see the differences.Examples:Aqueous SolutionHClhydrochloric acidHBrhydrobromic acidH2Shydrosulfuric acidHCNhydrocyanic acidHIhydroiodic acidNote: CN- is treated as if it were a single element.Gas Phasehydrogen chloridehydrogen bromidehydrogen sulfidehydrogen cyanidehydrogen iodideB. Bases: The OH- ion is considered as a single element, therefore all compoundscontaining OH- are called hydroxides.Example: Ca(OH)2NaOHNH3calcium hydroxidesodium hydroxideammonia (common name)C. Salts: If the metallic element has more than one valence, the oxidation number isdesignated by a Roman numeral: Fe(II) and Fe(III), for example. Group IA and IIAcations have only one valence; thus there is no need for a Roman numeral.D. Binary compounds containing two nonmetallic elements are usually named in thefollowing manner:The number of atoms each element in a chemical formula are indicated by numericalprefixes: mono (1), di (2), tri (3), tetra (4), penta (5), hexa (6), hepta (7), octa (8).Examples: N2Odinitrogen monoxideP2S5diphosphorous pentasulfide.10
II. Ternary CompoundsTernary compounds contain three elements.A. Acids: Most common ternary acids (also called oxyacids) contain hydrogen, oxygen,and another element.1. The most common acid consisting of this combination of elements is named byadding -ic to the nonmetallic element.Examples: H2SO4 sulfuric acidH3BO3 boric acidHClO3 chloric acidH2CO3 carbonic acidHNO3 nitric acidH3PO4 phosphoric acid2. For an acid containing one less oxygen atom than that in (1), the suffix -ic changesfrom -ic to -ous.Examples: H2SO3 sulfurous acidHClO2 chlorous acidHNO2 nitrous acidH3PO3 phosphorous acid3. For acids containing one less oxygen atom than in (2), the suffix remains the samebut the prefix hypo- is added.Example: HClO hypochlorous acid4. For acids containing one more oxygen atom than the most common acid with asuffix of –ic is named by adding the prefix per- to the name.Example: HClO4 perchloric acid5. A table has been prepared for you on the following page to help summarize thenomenclature rules for naming oxy-acids and oxy-anions. This table is not acomplete listing of all ternary compounds but it is a more visual summary of thesetypes of compounds and their corresponding names. The authors of this labmanual urge you to use it and expand it as necessary for your own needs.11
33PO43-Notice the shaded row. All of those anions are named using the –ate suffix only. Ifyou memorize those anions only, and know the nomenclature rules when oxygens areadded or removed, you will automatically know how to name them correctly withoutactually having to memorize them. A few examples are shown below.AnionNO2NO3ClO3ClOCO3SO32-NameNitrite ionNitrate ionChlorate ionHypochlorate ionCarbonate ionSulfite O3H2SO3NameNitric acidNitrous acidChloric acidHypochlorous acidCarbonic acidSulfurous acidRemember: Learn the “-ates” for both categories (how many oxygens and thecharge of the ion) and you will be able to name all the rest by only having to knowthe prefix and suffix.12
6. There are six strong acids that you need to memorize. This list can also befound in your current text book as well. Assume all other acids are weak acids.NameHydrochloric acidHydrobromic acidHydroiodic acidNitric acidPerchloric acidSulfuric acidStrong acidHClHBrHIHNO3HClO4H2SO4B. Salts:1. Anions of salts derived from the ic acids, with all hydrogens removed, are namedby changing ic to ate.Example: H2SO4 sulfuric acidNa2SO4 sodium sulfate.2. Anions of salts formed from acids containing an ous suffix are named by changingous to ite.Example: HClO2 chlorous acid NaClO2 sodium chlorite3. Anions of salts of hypo .ous acids retain the prefix hypo but ous is changed to ite.Example: HClO hypochlorous acid NaClO sodium hypochorite4. Anions of salts from a per.ic acid retain the prefix per and ate is substituted for ic.Example: HClO4 perchloric acidKClO4 sodium perchlorate.5. Some salts contains anions that contain hydrogen, e.g. KHS and NaHSO4. Theseanions are derived from acids which are not completely neutralized. The name ofthe anion is formed by adding the word “hydrogen” with a numerical prefix wherenecessary, to indicate the number of replaceable hydrogens. The word hydrogenoccurs first.Examples: NaHSO4Al(HSO4)3NaH2PO4Ca(H2PO4)2sodium hydrogen sulfatealuminum hydrogen sulfatesodium dihydrogen phosphatecalcium dihydrogen phosphateThe prefix “mono” is not necessary to indicate one hydrogen.Appendix 1 has many practice problems for you to work.13
Experiment 1Chemical Reactions and Net Ionic EquationsI. Objective:To predict the products of some displacement reactions and write net ionic equations.II. Chemical Principles:A. Reaction Types.Chemical reactions can be classified into several different categories. The commonclassifications are as follows:Note: For ease of production in this syllabus (aq) has been eliminated from all equationswhile (s), (l) and (g) have been used to represent phases. When you write chemicalreactions in your lab reports you must show all phases including (aq).1. Combination. This reaction type involves the combining of elements and/orcompounds to form a new compound.element2 Mg(s) element O2(g) elementO2(g) compound compound2 NO(g) 2 NO2(g)compoundNH3(g) compound compoundHBr(g) NH4Br(s)compound2 MgO(s)2. Decomposition. This reaction type involves the splitting apart of a single compoundto form new compounds or elements.compound2 KClO3(s) new compound and/or elements2 KCl(s) 3 O2(g)CaCO3(s) CaO(s) CO2(g)3. Single Replacement. This reaction type involves an element displacing anotherelement or ion in a compound, or a chemical compound displacing an element or ionfrom another compound.elementa Zn(s) compounda elementb2 HCl H2(g)14 compoundbZnCl2(s)
Cl2(g) 2 NaI I2 2 NaCl4. Double Displacement (Metathesis). This reaction type involves the exchange ofelements or ions in two compounds.compounda compoundb compoundc compoundda. precipitation:AgNO3 NaBr AgBr(s) NaNO3b. dissolutionCuO(s) 2 HCl H2O(l) CuCl2c. neutralizationHNO3 NH3 NH4NO35. Acid-Base Reactions. These reactions are commonly displacement reactions. To beable to predict such a reaction, you must know the identity and properties of a fewspecific acids and bases.Acids1. Strong Acids. All strong acids completely dissociate in water, for example:HClO4, HCl, HBr, HI, HNO3, H2SO4a. nitric acid:HNO3 H2O(l) H3O NO3b. sulfuric acid:H2SO4 H2O(l) H3O HSO4HSO4- H2O(l)H3O SO42The first ionization step for sulfuric acid is 100%, however the second step is anequilibrium situation and ionization is only partial.Note: Molecules of strong acids such as HClO4 and H2SO4 do not exist in solutionbecause we treat them as ionizing 100 %, that is as strong electrolytes. H (aq) can bewritten in place of H3O , the hydronium ion.15
2. Weak Acids. These acids react only slightly with water to produce the hydroniumion. They, however, will react completely with a strong base.AcidReactionacetic acidcarbonicacidammoniumionHC2H3O2 H2O(l)H2CO3 H2O(l)HCO3- H2O(l)NH4 H2O(l)H3O C2H3O2H3O HCO3H3O CO32H3O NH3Extent ofReaction0.42%0.065%0.0024%Bases1. Strong bases: dissociate completely in water.a. Soluble metal hydroxides. MOH M OHb. Insoluble metal hydroxides. All insoluble metal hydroxide dissolve to a verylimited extent to form metal ions and hydroxide ions. Because the dissolved formof the insoluble metal hydroxide dissociates completely it is considered a strongelectrolyte and thus it is a strong base. The OH- ion is the strongest base that existsin water. For example, calcium hydroxide is said to be insoluble, but the reality isthat some calcium and hydroxide ions exist in solution and therefore the solution isCa2 2 OHbasic. Ca(OH)2(s)Moderately soluble bases are strong bases because what does dissolve,dissociates 100%.2. Weak bases: These substances react slightly with water to produce OH- and areweak electrolytes.BaseReactionammoniaacetate ioncarbonateionfluorideion*1.0 M solutionNH3 H2OC2H3O2- H2OCO32- H2ONH4 OHHC2H3O2 OHHCO3- OH-Extent ofreaction*1.3%0.42%0.0024%F-HF OH-0.00039% H2O16
Salts:Salts contain a metal ion and a nonmetal or polyatomic anion. Salts can be formed by aneutralization reaction: a reaction between an acid and a base producing a salt and water.For example:NaOH HFNaF H2O(l)Ba(OH)2 H2SO4BaSO4(s) 2H2O(l)Some salts, such as sodium fluoride, are very soluble in water, therefore a change is notobserved upon reaction. However, some salts such as barium sulfate are quite insolublein water and a precipitate will be observed when formed as a product in a reaction.B. Predicting Products of Displacement Reactions and Writing Net Ionic Equations.To predict if a displacement reaction will occur, you must become familiar with theconditions required before a reaction takes place. Rules have been developed to assistyou with predicting the products of displacement reactions and for writing the net ionicequations associated with these reactions.You first determine if a displacement reaction can occur when you have two salts or anacid and base or a salt and acid/base reacting. Assume that a single or doubledisplacement is responsible for causing a reaction. Carry out the single or doubledisplacement reaction and focus on the predicted products. A product of a reactionhaving one of the characteristics in Table I supports the occurrence of a displacementreaction.Table I. Observations of a Chemical Reaction1.A A solid (precipitate) forms. This requires that you know thesolubility rules.2.A A new weak electrolyte or a compound with a new covalent bondforms. For example; formation of water, acetic acid, or carbondioxide.3.A A new gas forms. For example; the formation of gaseous water,carbon dioxide, hydrogen sulfide, hydrogen, or ammonia.4.A A new element forms. Zn, Pb, H2, O2 etc.5.A A precipitate dissolves. A colored, or clear, solution may result.Unless a precipitate forms, a gas evolves, or a colored ion forms, it may be difficult todetermine with your senses if a displacement reaction has taken place. Examples ofphysical evidence that sometime accompany a displacement reaction and which mayindicate their occurrences are: change in acidity or basicity of the product compared to the reactants.evolution or absorption of heat, other than heat of solution.solid reactant disappears.17
change in the color of the solution.precipitate forms in a solution.To apply these rules (1A -5A) you need to know which substances are strong and weakelectrolytes and which substances are soluble and insoluble and what is the limit ofsolubility of a compound in aqueous solution. Some rules are given in the followingTables.Table II. Strong and Weak Electrolytes1.B Strong electrolytes include all ionic substances except the halides andcyanides of Hg22 , Cd2 , Zn2 , and Ag . Strong acids, strong bases and manysalts are strong electrolytes.*2.B Weak electrolytes include weak acids, weak bases and many organiccompounds. Only a few ions will be produced in aqueous solution.3.BNonelectrolytes include pure water and many organic compounds,including sugar, for example. These are normally molecular compounds.* Many salts are insoluble in water, however, what limited quantity that does dissolve inwater, dissociates 100%. Salts, soluble or insoluble (except for those identified in 1B)will be treated as strong electrolytes. The terms strong electrolyte and solubility are notequivalent.Table III. Solubility Rules for Salts.1.C All alkali metal and ammonium compounds are soluble. KClO4 is slightlysoluble.2.C All nitrates are soluble.3.C All acetate salts are soluble. AgC2H3O2 is slightly soluble.4.C All sulfate salts are soluble except BaSO4, PbSO4, and Hg2SO4. Slightlysoluble salts include CaSO4, and SrSO4.5.C All salts of chloride, bromide, and iodide are soluble except those of Ag ,Pb2 , and Hg22 .6. C All hydroxides, phosphates, carbonates, chromates, oxalates and sulfidesare insoluble except those of the alkali metals and ammonium ion. Ba(OH)2,Ca(OH)2, and Sr(OH)2 are moderately soluble.7.C All oxides are quite insoluble.Note: If a compound is slightly soluble, usually it can be considered insoluble.It is necessary to know the solubility limit of a particular compound.Solubility is defined as the maximum amount of substance that dissolves in a givenamount of solvent at a given temperature . The solubility limit of many compounds canbe found in the Handbook. of Chemistry and Physics.18
C. Rules for Writing Net Ionic Equations1. Write the overall balanced “molecular” equation.2. Rewrite the molecular equation so that only soluble, strong electrolytes are separatedinto their ions.3. Eliminate all species common to the reactants and products (spectator ions).4. The resultant equation is the net ionic equation.5. There is no net ionic equation if there is no reaction.D. Application of Net Ionic Equation Rules.Example 1: (Production of a solid)Predict the outcome of the following reaction and write the net ionic equation,MgCl2 K2CO3 ?a. Complete the equation by carrying out a double replacement reaction (exchangepartners)MgCl2 K2CO3 2 KCl MgCO3b. Use rules 1.A - 6.A, 1.B - 3.B, and 1.C - 7.C to determine if a reaction occurred.According to 6.C, MgCO3 is insoluble and will precipitate. Ac
Experiment 9 Determination of Enthalpy and Entropy Changes 83 Experiment 10 Electrochemistry 88 Experiment 11 Sulfide Separations 99 Experiment 12 Separation and Identification Using Paper Chrom. 104 Experiment 13 Cis and Trans K[Cr(H2O)2(C2O4)2] 110 Experiment 14 Coordination Complexes of Co(III) 116
Chemistry ORU CH 210 Organic Chemistry I CHE 211 1,3 Chemistry OSU-OKC CH 210 Organic Chemistry I CHEM 2055 1,3,5 Chemistry OU CH 210 Organic Chemistry I CHEM 3064 1 Chemistry RCC CH 210 Organic Chemistry I CHEM 2115 1,3,5 Chemistry RSC CH 210 Organic Chemistry I CHEM 2103 1,3 Chemistry RSC CH 210 Organic Chemistry I CHEM 2112 1,3
Accelerated Chemistry I and Accelerated Chemistry Lab I and Accelerated Chemistry II and Accelerated Chemistry Lab II (preferred sequence) CHEM 102 & CHEM 103 & CHEM 104 & CHEM 105 General Chemistry I and General Chemistry Lab I and General Chemistry II and General Chemistry Lab II (with advisor approval) Organic chemistry, select from: 9-10
Physical chemistry: Equilibria Physical chemistry: Reaction kinetics Inorganic chemistry: The Periodic Table: chemical periodicity Inorganic chemistry: Group 2 Inorganic chemistry: Group 17 Inorganic chemistry: An introduction to the chemistry of transition elements Inorganic chemistry: Nitrogen and sulfur Organic chemistry: Introductory topics
2. CHE 133, CHE 134 General Chemistry Lab I, II or CHE 154 Molecular Science Laboratory I 3. CHE 301, CHE 302 Physical Chemistry I, II 4. CHE 303 Solution Chemistry Laboratory 5. CHE 321, CHE 322 Organic Chemistry I, II, or CHE 331, CHE 332 Molecular Science II, III 6. CHE 375 Inorganic Chemistry I 7.
CHEM 0350 Organic Chemistry 1 CHEM 0360 Organic Chemistry 1 CHEM 0500 Inorganic Chemistry 1 CHEM 1140 Physical Chemistry: Quantum Chemistry 1 1 . Chemistry at Brown equivalent or greater in scope and scale to work the studen
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Chemistry is the science that describes matter, its properties, the changes it undergoes, and the energy changes that accompany those processes. Inorganic chemistry Organic chemistry Physical chemistry Biochemistry Applied Chemistry: Analytical chemistry, Pharmaceutical Chemistry, . Istv an Szalai (E otv os University) Lecture 1 6 / 45
1 Chemistry 104: General Chemistry II Spring 2018, Section 004 Credits: Chemistry 104 is a 5-credit course. Whole-class meetings: TR 2:30 pm – 3:45 pm in Chemistry Building 1351 (150 minutes per week) Discussion meetings: Times, locations vary by discussion section (two 50-minute classes/week) Laboratory meetings: Times, locations vary by lab section (one 3-hour lab/week; 10 labs/semester)
